3) Consider the following reaction: 2 NOCI(g) 2 NO(g) + Cl₂(g) at T=450. K AH+75. kl/mol (3.1) A system initially contains NOCI, NO, and Cl, and is at equilibrium. For each of the following changes, indicate (by circling your answer) whether the number of moles of Ch in the system will increase, stay the same, or decrease. a) Add 0.100 moles of NOCI(g) to the system moles of Cl₂ moles of Cha will increase will not change b) Decrease the volume by 1.00 L moles of Ch will increase moles of Ch will not change c) Increase the temperature to T-500. K moles of Cl will increase moles of Ch will not change moles of Ch will decrease moles of Ch will decrease moles of Ch will decrease
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
I need help with letter C from question 3.
![### Consider the following reaction:
\[ 2 \text{NOCl(g)} \rightleftharpoons 2 \text{NO(g)} + \text{Cl}_2\text{(g)} \]
at \( T = 450 \, \text{K} \)
\( \Delta H^\circ_{\text{rxn}} = + 75 \, \text{kJ/mol} \)
A system initially contains NOCl, NO, and Cl₂, and is at equilibrium. For each of the following changes, indicate (by circling your answer) whether the number of moles of Cl₂ in the system will increase, stay the same, or decrease.
a) **Add 0.100 moles of NOCl(g) to the system**
- Moles of Cl₂ will increase (circled)
- Moles of Cl₂ will not change
- Moles of Cl₂ will decrease
b) **Decrease the volume by 1.00 L**
- Moles of Cl₂ will increase
- Moles of Cl₂ will not change
- Moles of Cl₂ will decrease (circled)
c) **Increase the temperature to \( T = 500 \, \text{K} \)**
- Moles of Cl₂ will increase
- Moles of Cl₂ will not change
- Moles of Cl₂ will decrease](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F929019dd-c141-42cd-9b2b-60111de8474f%2F02ee7030-1221-4d90-a798-e1d2ff24ed82%2Fyx3qo1_processed.jpeg&w=3840&q=75)
Answer:
Le Chatalier's principle states that on changing any parameter of the system in equilibrium, it will shift in the direction where effect of that change can get eliminated.
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